10/1/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 2. Chemistry: Atoms, Molecules and Ions

Size: px
Start display at page:

Download "10/1/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 2. Chemistry: Atoms, Molecules and Ions"

Transcription

1 General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy Chapter 2 Chemistry: Atoms, Molecules and Ions 1

2 The Structure of the Atom Dalton s Atomic Theory (1808) o Compounds are composed of atoms of more than one element. o Elements are composed of extremely small particles called atoms. o A chemical reaction involves only the separation, combination, or rearrangement of atoms; it does not result in their creation or destruction. The Structure of the Atom Dalton s Atomic Theory (1808) o Atom is the basic unit of an element that can enter into chemical combination. o Dalton imagined an atom that was both extremely small and indivisible. o The 1850s and extended into the twentieth century: atoms actually possess internal structure; they are made up of even smaller particles, which are called subatomic particles. o This research led to the discovery of three such particles - electrons, protons, and neutrons. 2

3 The Structure of the Atom The Electron o Radiation -theemission and transmission of energy through space in the form of waves. o One device used to investigate this phenomenon was a cathode ray tube (It is a glass tube from which most of the air has been evacuated). The Electron The Structure of the Atom When the two metal plates are connected to a high-voltage source; o The negatively charged plate, called the cathode, emits an invisible ray. o The cathode ray is drawn to the positively charged plate, called the anode, where it passes through a hole and continues traveling to the other end of the tube. o When the ray strikes the specially coated surface, it produces a strong fluorescence, or bright light. 3

4 The Electron The Structure of the Atom In some experiments, two electrically charged plates and a magnet were added to the outside of the cathode ray tube. o When the magnetic field is on and the electric field is off, the cathode ray strikes point A. o When only the electric field is on, the ray strikes point C. o When both the magnetic and the electric fields are off or when they are both on but balanced so that they cancel each other s influence, the ray strikes point B. According to electromagnetic theory, a moving charged body behaves like a magnet and can interact with electric and magnetic fields through which it passes. The Structure of the Atom The Electron o Because the cathode ray is attracted by the plate bearing positive charges and repelled by the plate bearing negative charges, it must consist of negatively charged particles. o We know these negatively charged particles as electrons. J.J. Thomson, measured mass/charge of e - (1906 Nobel Prize in Physics) Thomson s charge/mass of e - = x 10 8 C/g 4

5 The Structure of the Atom Millikan s Experiment Measured mass of e - (1923 Nobel Prize in Physics) o Millikan examined the motion of single tiny drops of oil that picked up static charge from ions in the air. o He suspended the charged drops in air by applying an electric field and followed their motions through a microscope. e - charge = x C Thomson s charge/mass of e - = x 10 8 C/g e - mass = 9.10 x g Radioactivity The Structure of the Atom o It was suggested by Marie Curie. o Radioactivity - spontaneous emission of particles and/or radiation. o Radioactive - any element that spontaneously emits radiation. o Röntgen noticed that cathode rays caused glass and metals to emit very unusual rays. Highly energetic radiation penetrated matter, darkened covered photographic plates, and caused a variety of substances to fluoresce. These rays could not be deflected by a magnet, they could not contain charged particles as cathode rays do. Röntgen called them X rays because their nature was not known. 5

6 The Structure of the Atom Radioactivity Three types of rays are produced by the decay, or breakdown, of radioactive substances such as uranium. 1.Two of the three are deflected by oppositely charged metal plates. o Alpha ( ) rays or particles; positively charged particles, and are deflected by the positively charged plate. o Beta ( ) rays or particles; are electrons and are deflected by the negatively charged plate. 2. Gamma ( ) rays; high-energy rays. Like X rays, rays have no charge and are not affected by an external field. The Structure of the Atom The Proton and the Nucleus o By the early 1900s, two features of atoms had become clear: they contain electrons, and they are electrically neutral. o To maintain electric neutrality, an atom must contain an equal number of positive and negative charges. Thomson s Model a uniform, positive sphere of matter in which electrons are embedded like raisins in a cake. This so-called plum-pudding model was the accepted theory for a number of years. 6

7 The Structure of the Atom The Proton and the Nucleus Rutherford s Experiment (1908 Nobel Prize in Chemistry) particle velocity ~ 1.4 x 10 7 m/s (~5% speed of light) 1. atoms positive charge is concentrated in the nucleus 2. proton (p) has opposite (+) charge of electron (-) 3. mass of p is 1840 x mass of e - (1.67 x g) The Structure of the Atom The Proton and the Nucleus Rutherford s Model of the Atom o Most of the atom must be empty space. This explains why the majority of a particles passed through the gold foil with little or no deflection. o The atom s positive charges, are all concentrated in the nucleus, which is a dense central core within the atom. o Whenever an particle came close to a nucleus in the scattering experiment, a large repulsive force and therefore a large deflection. o The positively charged particles in the nucleus are called protons. atomic radius ~ 100 pm = 1 x m nuclear radius ~ 5 x 10 3 pm = 5 x m 7

8 The Structure of the Atom The Neutron Chadwick s Experiment (1932) (1935 Noble Prize in Physics) o When a thin sheet of beryllium was bombarded with a particles, a very high-energy radiation similar to rays was emitted by the metal. o Later experiments showed that the rays actually consisted of a third type of subatomic particles, which Chadwick named neutrons, electrically neutral particles having a mass slightly greater than that of protons. H atoms - 1 p; He atoms - 2 p mass He/mass H should = 2 measured mass He/mass H = 4 neutron (n) is neutral (charge = 0) n mass ~ p mass = 1.67 x g The Neutron The Structure of the Atom mass p mass n 1840 x mass e - 8

9 Atomic Number, Mass Number and Isotopes Atomic number (Z) = number of protons in nucleus Mass number (A) = number of protons + number of neutrons = atomic number (Z) + number of neutrons Isotopes are atoms of the same element (X) with different numbers of neutrons in their nuclei Mass Number Atomic Number 1 H 2 A ZX 1 1H (D) 1H (T) U 92 U 235 Element Symbol hydrogen deuterium tritium Atomic Number, Mass Number and Isotopes The Isotopes of Hydrogen 9

10 Atomic Number, Mass Number and Isotopes 14 How many protons, neutrons, and electrons are in 6 C? 6 protons, 8 (14-6) neutrons, 6 electrons 11 How many protons, neutrons, and electrons are in 6 C? 6 protons, 5 (11-6) neutrons, 6 electrons Atomic Number, Mass Number and Isotopes 10

11 The Periodic Table Alkali Metal Alkali Earth Metal Period Group Halogen Noble Gas The Periodic Table Chemistry In Action Natural abundance of elements in Earth s crust Natural abundance of elements in human body 11

12 Molécules and Ions o A molecule is an aggregate of two or more atoms in a definite arrangement held together by chemical forces. H 2 H 2 O NH 3 CH 4 o A diatomic molecule contains only two atoms H 2, N 2, O 2, Br 2, HCl, CO diatomic elements o A polyatomic molecule contains more than two atoms O 3, H 2 O, NH 3, CH 4 Molécules and Ions o An ion is an atom, or group of atoms, that has a net positive or negative charge. cation ion with a positive charge If a neutral atom loses one or more electrons it becomes a cation. Na 11 protons 11 electrons Na + 11 protons 10 electrons anion ion with a negative charge If a neutral atom gains one or more electrons it becomes an anion. Cl 17 protons 17 electrons Cl - 17 protons 18 electrons 12

13 Molécules and Ions o A monatomic ion contains only one atom Na +, Cl -, Ca 2+, O 2-, Al 3+, N 3- o A polyatomic ion contains more than one atom OH -, CN -, NH 4+, NO 3 - Molécules and Ions Common Ions Shown on the Periodic Table 13

14 Molécules and Ions How many protons and electrons are in Al? 13 protons, 10 (13 3) electrons 3+ How many protons and electrons are in Se? 34 protons, 36 (34 + 2) electrons Chemical Formulas 14

15 Chemical Formulas o A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance o An empirical formula shows the simplest whole-number ratio of the atoms in a substance molecular H 2 O C 6 H 12 O 6 O 3 empirical H 2 O CH 2 O O N 2 H 4 NH 2 o An allotrope is one of two or more distinct forms of an element. Oxygen (O 2 ) and ozone (O 3 ) are allotropes of oxygen. diamond and graphite are allotropes of carbon. Chemical Formulas o Ionic compounds consist of a combination of cations and an anions The formula is usually the same as the empirical formula The sum of the charges on the cation(s) and anion(s) in each formula unit must equal zero The ionic compound NaCl 15

16 Chemical Formulas The most reactive metals (green) and the most reactive nonmetals (blue) combine to form ionic compounds. Chemical Formulas o If the charges on the cation and anion are numerically different, we apply the following rule to make the formula electrically neutral: The subscript of the cation is numerically equal to the charge on the anion, and the subscript of the anion is numerically equal to the charge on the cation. Aluminum Oxide. The cation is Al 3+ and the oxygen anion is O 2-. The sum of the charges is 2(+3) + 3(-2) = 0. Thus, the formula for aluminum oxide is Al2O3. 16

17 Chemical Formulas Formula of Ionic Compounds 2 x +3 = +6 3 x -2 = -6 Al 2 O 3 Al 3+ O 2-1 x +2 = +2 2 x -1 = -2 CaBr 2 Ca 2+ Br - 1 x +2 = +2 1 x -2 = -2 Na 2 CO 3 Na + CO 2-3 Chemical Formulas 17

18 o Ionic Compounds Often a metal + nonmetal Anion (nonmetal), add ide to element name BaCl 2 K 2 O Mg(OH) 2 KNO 3 barium chloride potassium oxide magnesium hydroxide potassium nitrate o Transition metal ionic compounds indicate charge on metal with Roman numerals FeCl 2 2 Cl - -2 so Fe is +2 iron(ii) chloride FeCl 3 3 Cl - -3 so Fe is +3 iron(iii) chloride Cr 2 S 3 3 S -2-6 so Cr is +3 (6/2) chromium(iii) sulfide 18

19 19

20 20

21 Molecular compounds They are usually composed of nonmetallic elements. Many molecular compounds are binary compounds. Naming binary molecular compounds is similar to naming binary ionic compounds. Weplacethenameofthefirstelementintheformulafirst,andthe second element is named by adding -ide to the root of the element name. HCl HBr SiC hydrogen chloride hydrogen bromide silicon carbide Molecular compounds If more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom 21

22 Molecular compounds HI NF 3 SO 2 N 2 Cl 4 NO 2 N 2 O hydrogen iodide nitrogen trifluoride sulfur dioxide dinitrogen tetrachloride nitrogen dioxide dinitrogen monoxide Molecular compounds Notes in naming compounds with prefixes: o The prefix mono- may be omitted for the first element. For example, PCl 3 is named phosphorus trichloride, not monophosphorus trichloride. o For oxides, the ending a in the prefix is sometimes omitted. For example, N 2 O 4 may be called dinitrogen tetroxide rather than dinitrogen tetraoxide. 22

23 23

24 Naming Acids Acids and Bases o An acid can be defined as a substance that yields hydrogen ions (H + ) when dissolved in water. For example: HCl gas and HCl in water o Pure substance, hydrogen chloride o Dissolved in water (H 3 O + and Cl ), hydrochloric acid o Anions whose names end in -ide form acids with a hydro- prefix and an -ic ending. HCl HCl hydrogen chloride hydrochloric acid Naming Acids Acids and Bases 24

25 Acids and Bases Naming Oxoacids and Oxoanions o An oxoacid is an acid that contains hydrogen, oxygen, and another element. HNO 3 nitric acid H 2 CO 3 carbonic acid H 3 PO 4 phosphoric acid Acids and Bases Naming Oxoacids and Oxoanions o The formulas of oxoacids are usually written with the H first, followed by the central element and then O. H 2 CO 3 HClO 3 HNO 3 H 3 PO 4 H 2 SO 4 carbonic acid chloric acid nitric acid phosphoric acid sulfuric acid 25

26 Acids and Bases Naming Oxoacids and Oxoanions Two or more oxoacids have the same central atom but adifferent number of O atoms; the following rules to name these compounds. 1. Addition of one O atom to the -ic acid: The acid is called per.. -ic acid. HClO 3 chloric acid HClO 4 perchloric acid 2. Removal of one O atom from the -ic acid: The acid is called -ous acid. HNO 3 nitric acid HNO 2 nitrous acid 3. Removal of two O atoms from the -ic acid: Theacidiscalled hypo... -ous acid. HBrO 3 Bromic acid HBrO hypobromous acid. Naming Oxoacids and Oxoanions o The rules for naming oxoanions, anions of oxoacids, are as follows: 1. When all the H ions are removed from the -ic acid, the anion s name ends with -ate. 2. When all the H ions are removed from the -ous acid, the anion s name ends with -ite. 3. The names of anions in which one or more but not all the hydrogen ions have been removed must indicate the number of H ions present. For example: H 3 PO 4 phosphoric acid H 2 PO - 4 dihydrogen phosphate HPO 2-4 hydrogen phosphate PO 3-4 phosphate 26

27 Naming Oxoacids and Oxoanions Naming Oxoacids and Oxoanions 27

28 Naming Bases Acids and Bases o A base can be defined as a substance that yields hydroxide ions (OH - ) when dissolved in water. NaOH KOH Ba(OH) 2 sodium hydroxide potassium hydroxide barium hydroxide 28

29 o Hydrates are compounds that have a specific number of water molecules attached to them. BaCl 2 2H 2 O LiCl H 2 O MgSO 4 7H 2 O Sr(NO 3 ) 2 4H 2 O barium chloride dihydrate lithium chloride monohydrate magnesium sulfate heptahydrate strontium nitrate tetrahydrate CuSO 4 5H 2 O CuSO 4 Familiar Inorganic Compounds 29

Atoms, Molecules and Ions

Atoms, Molecules and Ions Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small

More information

Atoms, Molecules and Ions

Atoms, Molecules and Ions Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small

More information

Atoms, Molecules, and Ions

Atoms, Molecules, and Ions Atoms, Molecules, and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small

More information

Formulas and Models 1

Formulas and Models 1 Formulas and Models 1 A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance An empirical formula shows the simplest whole-number ratio of the atoms in

More information

Molecules and Compounds

Molecules and Compounds Molecules and Compounds ed. Brad Collins Some images Copyright The McGraw-Hill Companies, Inc. A molecule is an aggregate of two or more atoms in a definite arrangement held together by chemical bonds

More information

Chapter 2. Atoms, Molecules, and Ions

Chapter 2. Atoms, Molecules, and Ions Chapter 2 Atoms, Molecules, and Ions The atomic theory Topics The structure of the atom Atomic number, mass number and isotopes The Periodic Table The atomic mass scale and the average atomic mass Molecules

More information

Ch 2: Atoms, Molecules, and Ions

Ch 2: Atoms, Molecules, and Ions AP Chemistry: Atoms, Molecules, and Ions Lecture Outline 2.1 The Atomic Theory of Matter Greek philosophers: Can matter be subdivided into fundamental particles? Democritus (460 370 BC): All matter can

More information

2.1 Atomic Theory of Matter

2.1 Atomic Theory of Matter Chapter 2 2.1 Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter re-emerged in the early nineteenth century, championed by John Dalton. Law of Conservation of Mass

More information

Chapter 2. Atoms, Molecules, and Ions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO

Chapter 2. Atoms, Molecules, and Ions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO Lecture Presentation Chapter 2 John D. Bookstaver St. Charles Community College Cottleville, MO Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter reemerged in

More information

Lecture Presentation. Chapter 2. Atoms, Molecules, and Ions. James F. Kirby Quinnipiac University Hamden, CT Pearson Education, Inc.

Lecture Presentation. Chapter 2. Atoms, Molecules, and Ions. James F. Kirby Quinnipiac University Hamden, CT Pearson Education, Inc. Lecture Presentation Chapter 2 James F. Kirby Quinnipiac University Hamden, CT Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter reemerged in the early nineteenth

More information

Chapter 2 Atoms, Molecules, and Ions semester 1/ The Structure of Atom 2.3 Atomic Number, Mass Number, and Isotopes 2.4 The Periodic Table

Chapter 2 Atoms, Molecules, and Ions semester 1/ The Structure of Atom 2.3 Atomic Number, Mass Number, and Isotopes 2.4 The Periodic Table Chapter 2 Atoms, Molecules, and Ions semester 1/2016 2.2 The Structure of Atom 2.3 Atomic Number, Mass Number, and Isotopes 2.4 The Periodic Table 2.5 Molecules and Ions 2.6 Chemical Formulas Ref: Raymond

More information

Chapter 2. Law of Definite Proportions. Law of Definite Proportions. Law of Conservation of Mass 10/7/2011 WATER H 2 O

Chapter 2. Law of Definite Proportions. Law of Definite Proportions. Law of Conservation of Mass 10/7/2011 WATER H 2 O Chapter 2 Fundamental Chemical Laws (2.2) Dalton s Atomic Theory (2.3) Defining the Atom (2.5) Atomic Structure (2.6) Molecules and Ions (2.7) The Periodic Table (2.8) Nomenclature (2.9) Law of Conservation

More information

Chapter 2. Chapter 2 Atoms, Molecules and Ions

Chapter 2. Chapter 2 Atoms, Molecules and Ions Chapter 2 Atoms, Molecules and Ions How can we classify these substances? What are their distinguishing characteristics? Can we classify them simply on the basis of appearance? 2.1 Atomic Theory How do

More information

Atomic Theory of Matter

Atomic Theory of Matter Chapter 2: Atoms, Molecules, and Ions Learning outcomes: Learn the basic postulates of Dalton s atomic theory. Describe the key experiments that led to the discovery of electrons and the nuclear model

More information

Law of Multiple Proportions Elements are composed of small particles,

Law of Multiple Proportions Elements are composed of small particles, CHAPTER 2 Atoms, Molecules, and Ions 2.1 Atomic Theory Democritus (5th century BC) suggested that matter was made of small, indivisible particles, atomos John Dalton (1808) formulated modern atomic theory

More information

Chapter 2. and Ions. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten

Chapter 2. and Ions. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 2 John D. Bookstaver St. Charles Community College Cottleville, MO Atomic Theory of Matter

More information

Chapter 2. Atoms, Molecules, and Ions

Chapter 2. Atoms, Molecules, and Ions Chapter 2 Atoms, Molecules, and Ions Section 2.1 The Early History of Chemistry Early History of Chemistry Greeks were the first to attempt to explain why chemical changes occur. Alchemy dominated for

More information

H 2 O. Chapter 9 Chemical Names and Formulas

H 2 O. Chapter 9 Chemical Names and Formulas H 2 O Chapter 9 Chemical Names and Formulas Section 9.1 Naming Ions OBJECTIVES: Identify the charges on monatomic ions by using the periodic table, and name the ions. Section 9.1 Naming Ions OBJECTIVES:

More information

Chemical Nomenclature

Chemical Nomenclature Chemical Nomenclature! The first names for chemicals were common names: Sugar, quicklime, Epsom salts, milk of magnesia, gypsom, laughing gas Simple, but not practical, the tell us little about the chemicals

More information

Chapter 2. Atoms, Molecules, and Ions. Lecture Outline

Chapter 2. Atoms, Molecules, and Ions. Lecture Outline Chapter 2. Atoms, Molecules, and Ions Lecture Outline 2.1 The Atomic Theory of Matter Greek Philosophers: Can matter be subdivided into fundamental particles? Democritus (460 370 BC): All matter can be

More information

Chapter 5 Molecules and Compounds

Chapter 5 Molecules and Compounds Chapter 5 Molecules and Compounds 1 Chemical Formulas Atomic/Molecular Elements Ionic/Molecular Compounds Naming Ionic Compounds Naming Molecular Compounds Naming Acids Formula Mass Atomic / Molecular

More information

Chapter 2: Atomic Theory

Chapter 2: Atomic Theory Chapter 2: Atomic Theory all things are made of atoms - little particles that move around in perpetual motion, attracting each other when they are a little distance apart, but repelling upon being squeezed

More information

AP* Chapter 2. Atoms, Molecules, and Ions. Monday, September 16, 13

AP* Chapter 2. Atoms, Molecules, and Ions. Monday, September 16, 13 AP* Chapter 2 Atoms, Molecules, and Ions AP Learning Objectives LO 1.1 The student can justify the observation that the ratio of the masses of the constituent elements in any pure sample of that compound

More information

Atoms, Molecules and Ions. Chapter 2

Atoms, Molecules and Ions. Chapter 2 Atoms, Molecules and Ions Chapter 2 2.1 The Atomic Theory of Matter Democritus [460-370 BCE] Described tiny, indivisible particles Called them atomos Differed from Aristotle 17th century - idea of atoms

More information

Chapter 2. Atoms and the Periodic Table. Chemistry: Atoms First Julia Burdge & Jason Overby

Chapter 2. Atoms and the Periodic Table. Chemistry: Atoms First Julia Burdge & Jason Overby Chemistry: Atoms First Julia Burdge & Jason Overby Chapter 2 Atoms and the Periodic Table Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 2 Atoms and the

More information

Atoms, Molecules, and Ions

Atoms, Molecules, and Ions Atoms, Molecules, and Ions Atomic Theory of Matter Postulates of Dalton s Atomic Theory All matter is composed of indivisible atoms. An atom is an extremely small particle of matter that retains its identity

More information

Chapter 1. Study of chemistry Classification of Matter Properties of Mater Unit of Measurements Uncertainty of Measurements Dimensional Analysis

Chapter 1. Study of chemistry Classification of Matter Properties of Mater Unit of Measurements Uncertainty of Measurements Dimensional Analysis Chapter 1 Completed Chapter Study of chemistry Classification of Matter Properties of Mater Unit of Measurements Uncertainty of Measurements Dimensional Analysis Quiz Next Thurs- Problems taken from Book

More information

Atoms, Molecules, and Ions

Atoms, Molecules, and Ions Chapter 2 Atoms, Molecules, l and Ions Chapter 2 Table of Contents 2.1 The Early History of Chemistry 2.2 Fundamental Chemical Laws 23 2.3 Dalton s Atomic Theory 2.4 Early Experiments to Characterize the

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Ch. 2 Practice Test Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which formula/name pair is incorrect? 1) A) Fe2(SO4)3 iron(iii) sulfide

More information

CHAPTER 2: ATOMS, MOLECULES AND IONS. -matter (element) is composed of indivisible and indestructible particles termed atoms

CHAPTER 2: ATOMS, MOLECULES AND IONS. -matter (element) is composed of indivisible and indestructible particles termed atoms CHAPTER 2: ATOMS, MOLECULES AND IONS DALTON's ATOMIC THEORY -matter (element) is composed of indivisible and indestructible particles termed atoms -all atoms of the same element are identical. atoms of

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement

More information

Chapter 2. Atoms, Molecules, and Ions

Chapter 2. Atoms, Molecules, and Ions Chapter 2. Atoms, Molecules, and Ions 2.1 The Atomic Theory of Matter 400-5 BC. Greek philosopher Democritus proposes the idea of matter being made up of small, indivisible particles (atomos). 18th Century.

More information

Experiment #3: When 2.0 g of sodium hydroxide reacts with 2.2 g carbon dioxide, 4.2 g of baking soda (sodium bicarbonate) is produced.

Experiment #3: When 2.0 g of sodium hydroxide reacts with 2.2 g carbon dioxide, 4.2 g of baking soda (sodium bicarbonate) is produced. Name: Dalton s Atomic Theory: (1) Matter is composed of very small units called atoms. Atom is the smallest unit that possesses the chemical property of an element. (2) An element contains only one type

More information

Chapter 2. Chapter 2

Chapter 2. Chapter 2 Chapter 2 Atoms, Molecules, and Ions Chapter 2 Atomic Theory Model for atom and ions that works well for chemistry Molecules Combinations of atoms Ways of representing molecules: formulas and models Names

More information

Chemical Formulas & Chemical Compounds. Chemical formula indicates the relative number of atoms of each kind in a chemical compound.

Chemical Formulas & Chemical Compounds. Chemical formula indicates the relative number of atoms of each kind in a chemical compound. Unit 6: Chemical Formulas & Chemical Compounds Chemical Names & Formulas Chemical formula indicates the relative number of atoms of each kind in a chemical compound. Molecular compound - it s formula reveals

More information

Chapter 2 Atoms, Molecules, and Ions. 許富銀 ( Hsu Fu-Yin)

Chapter 2 Atoms, Molecules, and Ions. 許富銀 ( Hsu Fu-Yin) Chapter 2 Atoms, Molecules, and Ions 許富銀 ( Hsu Fu-Yin) 1 The Atomic Theory of Matter Democritus (460 370 bce) and other early Greek philosophers described the material world as made up of tiny, indivisible

More information

Nomenclature of inorganic compounds. = naming non carbon (mostly) compounds. Some definitions:

Nomenclature of inorganic compounds. = naming non carbon (mostly) compounds. Some definitions: 1 Chemistry 047 Inorganic Nomenclature Nomenclature of inorganic compounds = naming non carbon (mostly) compounds Some definitions: Nomenclature = system used by chemists to name and identify compounds

More information

Chapter 2: Atoms, Molecules, and Ions

Chapter 2: Atoms, Molecules, and Ions Chapter 2: Atoms, Molecules, and Ions 1. According to the law of definite proportions, A) the ratio of the masses of the elements in a compound is always the same. B) it is not possible for the same two

More information

CHEMISTRY 1: Chemical Bonding

CHEMISTRY 1: Chemical Bonding CHEMISTRY 1: Chemical Bonding Brown, T.L., LeMay, H.E., and B.E. Bursten. Chemistry: The Central Science 8 th Ed. New Jersey: PrenticeHall, 2002. CHEMICAL BONDS The forces that hold atoms or ions together

More information

Law of Definite Proportion** (Proust): A given compound always contains exactly the same proportion of elements by mass.

Law of Definite Proportion** (Proust): A given compound always contains exactly the same proportion of elements by mass. # 10 Notes Unit 2: Laws, Properties & Mols Ch. Atoms, Molecules, Ions 5 Chemical Laws: I. Law of Conservation of Mass** (Lavoisier): Mass cannot be created or destroyed. II. III. IV. Law of Definite Proportion**

More information

Chemistry CRT Study Guide First Quarter

Chemistry CRT Study Guide First Quarter Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry

More information

Chapter 2 Atoms, Molecules, and Ions

Chapter 2 Atoms, Molecules, and Ions 1. What name is given to the concept that different samples of a given compound always contain the same elements in the same mass ratio? A) Ration Law D) Law of Definite Proportions B) Law of Equality

More information

Chapter 6 and 15 Ionic Compounds

Chapter 6 and 15 Ionic Compounds Chapter 6 and 15 Ionic Compounds Chapter 6 Ionic compounds 6.3, 6.4 6.1: Intro to Chemical Bonding A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different

More information

4. What is the law of constant composition (also known as the law of definite proportion)?

4. What is the law of constant composition (also known as the law of definite proportion)? Name: Exercises #1: 1. What is the law of conservation of mass? 2. Show that the results of the following experiments illustrate the law of conservation of mass. Experiment #1: a 5.00-g sample of pure

More information

Chapter 2 Atoms and Elements

Chapter 2 Atoms and Elements Chapter 2 Atoms and Elements Law of Conservation of Mass in a chemical reaction, matter is neither created nor destroyed total mass of the materials you have before the reaction must equal the total mass

More information

Naming and Formula Writing

Naming and Formula Writing + Naming and Formula Writing + Chemical Formulas Shows the kind and number of atoms in the smallest piece of a substance Use subscripts to show the number of atoms per element Molecular formula- number

More information

DETERMINING THE FORMULA OF AN IONIC COMPOUND FROM THE NAME

DETERMINING THE FORMULA OF AN IONIC COMPOUND FROM THE NAME DETERMINING THE FORMULA OF AN IONIC COMPOUND FROM THE NAME - The name of an ionic compound is made of the names of the CATION and ANION in the compound. - To get the FORMULA, you must figure out the SMALLEST

More information

4.1 Structure of the Atom

4.1 Structure of the Atom 4.1 Structure of the Atom How do atoms differ from each other? What are atoms composed of? What are the subatomic particles? 2-1 Structure of the Atom Atoms actually are divisible. They are composed of

More information

Chemistry Chapter 2. Atoms, Molecules, and Ions Section Periodic Table Ions Chemical Bonds Nomenclature

Chemistry Chapter 2. Atoms, Molecules, and Ions Section Periodic Table Ions Chemical Bonds Nomenclature Chemistry Chapter 2 Atoms, Molecules, and Ions Section 2 2.6-2.8 Periodic Table Ions Chemical Bonds Nomenclature Organization of the Periodic Table Columns, Groups or Families elements in the same vertical

More information

Chapter 2: Atoms, Molecules, and Ions

Chapter 2: Atoms, Molecules, and Ions Download full Download Chemical Principles 7th Edition by Zumdahl Test Bank https://digitalcontentmarket.org/download/download-chemical-principles-7th-edition-by-zumdahl-te st-bank Chapter 2: Atoms, Molecules,

More information

CHEMA1301 Selected Questions Chapter 2

CHEMA1301 Selected Questions Chapter 2 CHEMA1301 Selected Questions Chapter 2 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of. A) the law of multiple proportions B) the law of constant composition

More information

Chapter 9. Chemical Names and Formulas

Chapter 9. Chemical Names and Formulas Chapter 9 Chemical Names and Formulas 9.1 - Naming Ions Monatomic ions: Single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons. - Cations: Groups

More information

This chapter deals with matter, in its various forms, on the nanoscale.

This chapter deals with matter, in its various forms, on the nanoscale. Chapter 2 (Hill/Petrucci/McCreary/Perry This chapter deals with matter, in its various forms, on the nanoscale. While we believe that all matter is composed of protons, electrons and, usually, neutrons,

More information

Chemical Nomenclature Chapter 2.5-8

Chemical Nomenclature Chapter 2.5-8 Chemical Nomenclature Chapter 2.5-8 Octet Rule An octet is 8 valence electrons is associated with the stability of the noble gases does not occur with He, which is stable with two valence electrons (duet)

More information

Chemistry--Unit 2: Chemical Names and Formulas Test Review

Chemistry--Unit 2: Chemical Names and Formulas Test Review vocab anion binary compound cation chemical formula formula unit ion ionic compound law of definite proportions law of multiple proportions molecular formula polyatomic ion representative particle ternary

More information

Chapter 2 Atoms, Molecules and Ions

Chapter 2 Atoms, Molecules and Ions Sec$on 2.1 The Early History of Chemistry Chapter 2 Atoms, Molecules and Ions Sec$on 2.1 The Early History of Chemistry Early History of Chemistry Greeks were the first to a?empt to explain why chemical

More information

The Components of Matter

The Components of Matter The Components of Matter Elements the basic building blocks of matter Ancient Greeks four elements: earth, air, fire and water The atomic idea Democritus there are atoms and void. Boyle (17 th century)

More information

Naming Chemical Compounds

Naming Chemical Compounds Naming Chemical Compounds Naming compounds is an important part of chemistry. Most compounds fall into one of four categories Ionic Compounds, Molecular Compounds, Acids and Bases, and Hydrates Part One:

More information

+ #n; Z = atomic number = #p + C isotopes: 12 6

+ #n; Z = atomic number = #p + C isotopes: 12 6 CHEMISTRY 103 Help Sheet #2 Chapter 2 (Part I); Sections 2.1.8 Do topics appropriate for your lecture Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets: Periodic Table;

More information

Atomic Theory of Matter

Atomic Theory of Matter Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter John Dalton (1766-1844) Postulates of Dalton s Theory 1) Each element is composed of extremely small particles

More information

Voltage source. Voltage source. Voltage source

Voltage source. Voltage source. Voltage source Chapter 2 Atoms, Molecules, and Ions History Greeks Democritus and Leucippus atomos Aristotle elements Alchemy 1660 Robert Boyle experimental definition of element. Lavoisier Father of modern chemistry

More information

AP Chemistry Chapter 2

AP Chemistry Chapter 2 AP Chemistry Chapter 2 Atoms, Molecules & Ions The Atomic Theory of Maer > Democritus (460 370 BC) > Greek philosopher > Thought that material was made up of ny indivisible parcles called atomos > Aristotle

More information

Chapter 2 Atoms, Molecules, and Ions

Chapter 2 Atoms, Molecules, and Ions hapter 2 Atoms, Molecules, and Ions 2.1 The Atomic Theory of Matter Is there such thing like a indivisible particle of matter (atom)? Based on the following observations: 1. Law of conservation of mass/matter

More information

Chapter 2 : Atoms, Molecules, and Ions

Chapter 2 : Atoms, Molecules, and Ions Chapter 2 : Atoms, Molecules, and Ions Parmenides (BC 515? BC 445?) : < 있는것 ( 토에온 )> 은있고 < 없는것 ( 토메에온 )> 은없다고하는전제 ( 前提 ) 에서불생불멸 불가분 불변부동이며, 완결된둥근공과비슷하다고하는 < 있는것 > 의속성을끌어내고, < 있는것 > 을우리에게보여주는이성만이진리를포착하며생성

More information

9.4 Naming and Writing. Formulas for Acids and Bases. Chapter 9 Chemical Names and Formulas. 9.4 Naming and Writing Formulas for Acids and Bases

9.4 Naming and Writing. Formulas for Acids and Bases. Chapter 9 Chemical Names and Formulas. 9.4 Naming and Writing Formulas for Acids and Bases Chapter 9 Chemical Names and Formulas 9.1 Naming Ions 9.2 Naming and Writing Formulas for Ionic Compounds 9.3 Naming and Writing Formulas for Molecular Compounds 9.4 Naming and Writing Formulas for Acids

More information

AP CHEMISTRY THINGS TO KNOW

AP CHEMISTRY THINGS TO KNOW AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not

More information

Chemical Formulas Types of chemical formulas [X m Y n ]

Chemical Formulas Types of chemical formulas [X m Y n ] 1 Chemical Formulas Types of chemical formulas [X m Y n ] Molecular Actual # of atoms of each element Empirical Structural Relative # of atoms of each element Actual # of atoms and the bonds between them

More information

AP Chemistry (1 of 20) AP Chemistry (2 of 20) AP Chemistry (3 of 20) AP Chemistry (4 of 20) AP Chemistry (5 of 20) AP Chemistry (6 of 20)

AP Chemistry (1 of 20) AP Chemistry (2 of 20) AP Chemistry (3 of 20) AP Chemistry (4 of 20) AP Chemistry (5 of 20) AP Chemistry (6 of 20) Ions Ionic Charges of Representative Elements (1 of 20) (2 of 20) Formulas and Names of Common Metal Ions with More than One Common Ionic Charge Some Common Polyatomic Ions (3 of 20) (4 of 20) Naming Monatomic

More information

Chapter 2. Atoms and the Periodic Table. Chemistry: Atoms First Third Edition Julia Burdge and Jason Overby

Chapter 2. Atoms and the Periodic Table. Chemistry: Atoms First Third Edition Julia Burdge and Jason Overby Chemistry: Atoms First Third Edition Julia Burdge and Jason Overby Chapter 2 Atoms and the Periodic Table Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter

More information

Chapter 2: Atoms, Molecules and Ions

Chapter 2: Atoms, Molecules and Ions Chapter 2: Atoms, Molecules and Ions Sep 24 10:24 AM 2.1 The Early History of Chemistry The Greek did not use experiments to establish the veracity of their ideas. Alchemy "gold making juice" Khem the

More information

- Some MOLECULES can gain or lose electrons to form CATIONS or ANIONS. These are called POLYATOMIC IONS

- Some MOLECULES can gain or lose electrons to form CATIONS or ANIONS. These are called POLYATOMIC IONS 63 POLYATOMIC IONS - Some MOLECULES can gain or lose electrons to form CATIONS or ANIONS. These are called POLYATOMIC IONS - Polyatomic ions form ionic compounds in the same way that single-element ions

More information

Big Idea: Matter & Atoms

Big Idea: Matter & Atoms Big Idea: Matter & Atoms Naming Ionic Compounds Naming Covalent Compounds Naming Acids Naming Hydrates The cation (positive ion) is written first Takes the same name as the element if only forms one charge

More information

Atoms, Molecules and Ions

Atoms, Molecules and Ions Atoms, Molecules and Ions Atomic Theory of Matter Modern Atomic Theory Relation to Periodic Table Isotopes & Mass Number Periodic Table Ionic Compounds Molecular Compounds Acid Compounds The Atomic Theory

More information

NAMING IONIC COMPOUNDS. ammonium sulfide. iron(ii) carbonate. barium phosphate. titanium(iv) sulfide. Spelling matters!

NAMING IONIC COMPOUNDS. ammonium sulfide. iron(ii) carbonate. barium phosphate. titanium(iv) sulfide. Spelling matters! 67 NAMING IONIC COMPOUNDS ammonium sulfide iron(ii) carbonate titanium(iv) sulfide barium phosphate Spelling matters! barium phosphide 68 DETERMINING THE FORMULA OF AN IONIC COMPOUND FROM THE NAME - The

More information

NAMING IONIC COMPOUNDS

NAMING IONIC COMPOUNDS NAMING IONIC COMPOUNDS iron(ii) carbonate ammonium sulfide titanium (IV) sulfide barium phosphate Spelling matters! calcium nitrate sodium phosphide DETERMINING THE FORMULA OF AN IONIC COMPOUND FROM THE

More information

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms,

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms, Chemical Bonding Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that is that valence electrons are the

More information

Atoms, Molecules, and Ions

Atoms, Molecules, and Ions Atoms, Molecules, and Ions Chapter 2 Copyright McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of McGraw-Hill Education. Dalton s Atomic Theory

More information

Chapter 5. Naming Compounds Writing Formulas

Chapter 5. Naming Compounds Writing Formulas Chapter 5 Naming Compounds Writing Formulas Systematic Naming There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms. Name should tell

More information

What is the major difference between a molecular formula and formula unit?

What is the major difference between a molecular formula and formula unit? Lecture 5 Molecular Substances versus Ionic Substances Molecular Substance Ionic Substance What are some examples of molecular substances? What are some examples of ionic substances? What is the major

More information

Ionic Compounds. And Acids

Ionic Compounds. And Acids CHAPTER 7 LANGUAGE OF CHEMISTRY CLASSIFICATION OF COMPOUNDS Inorganic compounds does not contain the element carbon, but there are exception to this rule, CO 2 (carbon dioxide), CO 3 2 (carbonate), and

More information

Chapter 2. Atoms, Molecules, and Ions. Copyright 2017 Cengage Learning. All Rights Reserved.

Chapter 2. Atoms, Molecules, and Ions. Copyright 2017 Cengage Learning. All Rights Reserved. Chapter 2 Atoms, Molecules, and Ions Chapter 2 Table of Contents (2.1) (2.2) (2.3) (2.4) (2.5) (2.6) (2.7) (2.8) The early history of chemistry Fundamental chemical laws Dalton s atomic theory Early experiments

More information

CHAPTER 2. ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color. Questions

CHAPTER 2. ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color. Questions CHAPTER 2 ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color Questions 17. A compound will always contain the same numbers (and types) of atoms. A given amount of hydrogen will react only

More information

CHAPTER 4 Atomic Structure

CHAPTER 4 Atomic Structure CHAPTER 4 Atomic Structure 4.1 Early Theories of Matter Earth, Water, Air, Fire Matter was thought to be infinitely divisible No method was available to test theories Democritus (460 B.C. 370 B.C.) First

More information

CHEMISTRY 103 Help Sheet #2 Atoms, Molecules, and Ions (Text: Ch 2: )

CHEMISTRY 103 Help Sheet #2 Atoms, Molecules, and Ions (Text: Ch 2: ) CHEMISTRY 103 Help Sheet #2 Atoms, Molecules, and Ions (Text: Ch 2: 2.1-2.8) Do the topics appropriate for your lecture Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets:

More information

Chapter 6. Naming Compounds Writing Formulas

Chapter 6. Naming Compounds Writing Formulas Chapter 6 Naming Compounds Writing Formulas Systematic Naming There are too many compounds to remember the names of them all. Compound is made of two or more elements. Put together atoms. Name should tell

More information

Ch 2 Atoms, Molecules, and Ions

Ch 2 Atoms, Molecules, and Ions Ch 2 Atoms, Molecules, and Ions John Dalton s Atomic Theory (four postulates from1805) - An atom is the smallest particle with a chemical identity. Its identity is retained during chemical reactions. -

More information

Chapter 2 Atoms, Molecules, and Ions

Chapter 2 Atoms, Molecules, and Ions hapter 2: Phenomena Phenomena: Some elements, such as A and B, are known to form several compounds. Data on the masses of A and B were collected on different sample sizes of the three compounds. What patterns

More information

Naming and Counting Atoms and Molecules. Chemistry--Unit 2

Naming and Counting Atoms and Molecules. Chemistry--Unit 2 Naming and Counting Atoms and Molecules Chemistry--Unit 2 Masses of 22.4 L O 2, N 2, & HCl N 2 28 g O 2 32 g HCl 36.5 g Observation: At 1 atmosphere pressure and 0 o C, 22.4 L of 3 different gases have

More information

Unit 2. Atoms, Molecules, and Ions

Unit 2. Atoms, Molecules, and Ions Unit 2. Atoms, Molecules, and Ions Upon successful completion of this unit, the students should be able to: 2.1 State and be able to apply the Law of Conservation of Mass, Law of Definite Proportions,

More information

Chapter 2 Atoms and Elements

Chapter 2 Atoms and Elements 1 Chapter 2 Atoms and Elements Sec 2.3 Modern Atomic Theory and the Laws That Led to it Law of conservation of mass states that in a chemical reaction, matter is neither created nor destroyed. Law of definite

More information

(COMMON IONS AND THEIR CHARGES QUIZZES BEGIN)

(COMMON IONS AND THEIR CHARGES QUIZZES BEGIN) (COMMON IONS AND THEIR CHARGES QUIZZES BEGIN) Chapter 2 Homework Problems on Pages 70 75; Set 1: Watch Khan Academy videos at http://www.khanacademy.org/#chemistry Elements and Atoms, Introduction to the

More information

Chapter 9 Study Guide

Chapter 9 Study Guide Name: Class: Date: Chapter 9 Study Guide Matching Match each item with the correct statement below. a. monatomic ion f. cation b. acid g. binary compound c. base h. anion d. law of definite proportions

More information

4. The mass of a proton is approximately equal to the mass of A an alpha particle C a positron. B a beta particle D a neutron

4. The mass of a proton is approximately equal to the mass of A an alpha particle C a positron. B a beta particle D a neutron 1. Which particles have approximately the same mass? A an electron and an alpha particle B an electron and a proton C a neutron and an alpha particle D a neutron and a proton 2. Which phrase describes

More information

Naming Inorganic Compounds. common names systematic names

Naming Inorganic Compounds. common names systematic names Naming Inorganic Compounds common names systematic names Molecular Common Systematic Formula name name AgCl Lunar caustic Silver chloride H 2 SO 4 Oil of vitriol Sulfuric acid MgSO 4 Epsom salts Magnesium

More information

Mass Relationships in Chemical Reactions. Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn

Mass Relationships in Chemical Reactions. Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn Mass Relationships in Chemical Reactions Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn Example 3.6 (3) We now write, 6.07 g CH 4 1 mol CH 4 16.04 g CH 4 = 0.378 mol CH 4 Thus, there is 0.378 mole

More information

Bonding and Nomenclature notes.notebook

Bonding and Nomenclature notes.notebook Chemical Bonding & Nomenclature Objectives: Distinguish between covalent and ionic bonding Explain the process of bonding Name ionic and covalent compounds and acids Write chemical formulas for ionic and

More information

Atoms, Molecules, and Ions. Chapter 2 AP Chemistry

Atoms, Molecules, and Ions. Chapter 2 AP Chemistry Atoms, Molecules, and Ions Chapter 2 AP Chemistry Building blocks of chemistry. Atom Molecule Ion Dalton s Atomic Theory 1. An element is composed of tiny particles called atoms. 2. In an ordinary chemical

More information

Chapter 2 Atoms, Ions, and the Periodic Table. Law of Conservation of Mass. Law of Conservation of Mass

Chapter 2 Atoms, Ions, and the Periodic Table. Law of Conservation of Mass. Law of Conservation of Mass Chapter 2 Atoms, Ions, and the Periodic Table Dalton s Atomic Theory Structure of the Atom Ions Atomic Mass The Periodic Table Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction

More information

ACP Chemistry (821) - Mid-Year Review

ACP Chemistry (821) - Mid-Year Review ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference

More information

EIT Review S2007 Dr. J.A. Mack.

EIT Review S2007 Dr. J.A. Mack. EIT Review S2007 Dr. J.A. Mack www.csus.edu/indiv/m/mackj/ Part 1 Atom: The smallest divisible unit of an element Compound: A substance made of two or more atoms Ion: A charged atom or molecule Cation:

More information